how many mL of a .094 M NaOh are needed to neutralize 21.4 mL of .160 M HCL
HCl + NaOH ==> NaCl + HOH
moles HCl = M x L = ??
Using the coefficients in the balanced equation, convert moles HCl to moles NaOH.
Then M NaOH = moles NaOH/L NaOH and solve for L, then convert to mL.
To determine the number of mL of NaOH required to neutralize the given volume of HCl, we can use the concept of stoichiometry and the equation of the reaction between NaOH and HCl.
The balanced chemical equation for the reaction between NaOH and HCl is:
NaOH + HCl → NaCl + H2O
From the equation, we can see that the stoichiometric ratio between NaOH and HCl is 1:1, which means that one mole of NaOH reacts with one mole of HCl.
Now, let's calculate the number of moles of HCl in the given solution:
Number of moles of HCl = concentration of HCl × volume of HCl
= 0.160 M × 21.4 mL
= 3.424 millimoles (mmol)
Since the stoichiometry 1:1 ratio exists between NaOH and HCl, we need an equal number of moles of NaOH to neutralize the HCl.
Now, let's convert the number of moles of NaOH into the required volume of NaOH solution:
Number of moles of NaOH = Number of moles of HCl
= 3.424 mmol
To convert mmol to moles, divide by 1000:
Number of moles of NaOH = 3.424 mmol ÷ 1000
= 0.003424 moles
Now, let's calculate the volume of NaOH solution using its concentration:
0.003424 moles = concentration of NaOH × volume of NaOH (in liters)
Concentration of NaOH = 0.094 M (given)
Therefore,
0.003424 moles = 0.094 M × volume of NaOH (in liters)
Rearranging the equation, we get:
Volume of NaOH (in liters) = 0.003424 moles ÷ 0.094 M
= 0.03643 liters
Since we need the volume in milliliters (mL), we convert it back by multiplying by 1000:
Volume of NaOH (in mL) = 0.03643 liters × 1000
= 36.43 mL
Therefore, approximately 36.43 mL of a 0.094 M NaOH solution is needed to neutralize 21.4 mL of a 0.160 M HCl solution.